Light Practice Problems

Slides:

Advertisements

Similar presentations

Quantum Theory and the Electronic Structure of Atoms

Advertisements

What do you see? Old woman? Or young girl?  Is turning a light on and off a chemical or physical change? ◦ Physical change  What creates light?

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Inorganic chemistry Assistance Lecturer Amjad Ahmed Jumaa  Calculating the number of atoms in a given amount of a compound.  Calculating.

Wavelength, Frequency, and Energy Practice Problems

The Electromagnetic Spectrum Rainbows plus a whole lot more.

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Radiant Energy .

ENERGY & LIGHT THE QUANTUM MECHANICAL MODEL. Atomic Models What was Rutherford’s model of the atom like? What is the significance of the proton? What.

Instructions To use this template: –for each slide write the correct answer on the orange bar first –choose which option (A,B,C or D) and make sure you.

Properties of Light Is Light a Wave or a Particle?

Wave & Particle Nature of Light EQ: How can an atom be a "particle" and a "wave" at the same time?

wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Wave Nature of Light and Quantum Theory

Electronic Structure of Atoms

Electronic Structure. Wavelength ____________ (λ) - the shortest distance between equal points wave.

Electromagnetic Spectra Review Game. When do electrons emit light? Moving from higher to lower energy levels.

1 Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Quantum Theory and the Electronic Structure of.

Section 5.3 Physics and the Quantum Mechanical Model

Guiding Questions 1. How fast does light travel? How can this speed be measured? 2. Why do we think light is a wave? What kind of wave is it? 3. How is.

Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.

Chapter 4 Arrangement of Electrons in Atoms

Energy Levels & Photons Atomic & Nuclear Lesson 2.

Electronic Structure. Bohr Bohr proposed that the __________ atom has only certain allowable energy states.

Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Chapter 6 Electronic Structure of Atoms. The Wave Nature of Light The light that we can see with our eyes, visible light, is an example of electromagnetic.

Quantum Theory and the Electronic Structure of Atoms Chapter 7.

Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Light and the Atom. Light Much of what we know about the atom has been learned through experiments with light; thus, you need to know some fundamental.

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

Weird experiments Schrödinger equation.

Quantum Theory and the Electronic Structure of Atoms Chapter 6.

Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Light and Electrons! Ch 11. Light & Atomic Spectra A Brief Bit of History (development of the quantum mechanical model of the atom) Grew out of the study.

Electrons and Light. Light’s relationship to matter Atoms can absorb energy, but they must eventually release it When atoms emit energy, it is released.

LIGHT and QUANTIZED ENERGY. Much of our understanding of the electronic structure of atoms has come from studying how substances absorb or emit light.

c = 13.A mercury vapor lamp emits radiation with a wavelength of 4.36 x m. a.Use the wave equation to determine the frequency. = c Knowns and unknown.

STATION 1 Light and Waves 1.According to Einstein’s view of matter and energy, what is the common link between light and matter? 2.How does diffraction.

Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Wavelength, Frequency, and Planck’s Constant. Formulas 1)E = hf E = energy (Joules J) h = Planck’s constant = 6.63 x J x s f = frequency (Hz) 2)

© 2009, Prentice-Hall, Inc. The Nature of Energy Another mystery in the early 20th century involved the emission spectra observed from energy emitted by.

Using Planck’s Constant…. Picture credit: He was a German physicist and is considered as the founder.

Electrons in Atoms Chapter 4.

Warm-Up What is the difference between the Bohr’s Model of the Atom and the Quantum Model of the atom. What wavelength is associated with an electron.

Wave-Particle Nature of Light

Electrons in Atoms Chapter 4.

Chapter 6 Electronic Structure of Atoms

Light Ken Rogers Miami Killian.

II. Bohr Model of the Atom (p )

Why Light, why now?.

Atomic Structure the wave nature of light 1 2 3 2 Hz 4 Hz 6 Hz 

Bohr Model of the Atom College Chemistry.

Electromagnetic Radiation

Chapter 4 The Wave Description of Light

Sections 6.1 – 6.3 Electromagnetic Radiation and its Interaction with Atoms Bill Vining SUNY College at Oneonta.

Waves and Electromagnetic Radiation

Review Lepton Number Particle Lepton number (L) electron 1 neutrino

Waves and particles Ch. 4.

Light and the Electromagnetic Spectrum

Electronic Structure.

e–’s absorb (+) energy, move to outer levels

Quantum Theory.

Chapter 4 Arrangement of Electrons in Atoms

Quantum Physics – Photons Mr Nesbo

Electrons in Atoms C = fl.

Electromagnetic Spectrum

Chapter 6: Electromagnetic Radiation

Light and EM Spectrum Light is all thanks to electrons…well… photons…but whatever. What do you REALLY know about light?

Presentation transcript:

Light Practice Problems Ms. DiOrio

Equations On Equation Sheet NOT on Equation Sheet Planck’s Equation: 𝐸=ℎ𝜈 Wave Equation: 𝑐= 𝜆𝜈 Beer’s Law: A = abc E = energy 𝜈 = frequency 𝜆 = wavelength Planck’s Constant: h = 6.626 x 10-34 Js Speed of light: c = 3 x 108 m/s 𝐸= ℎ𝑐 𝜆 𝐸=𝑛ℎ𝜈 De Broglie Equation: λ= ℎ 𝑚𝑣 Bohr Equation: ∆𝐸=−2.178𝑥 10 −18 ( 1 𝑛 𝑓𝑖𝑛𝑎𝑙 2 − 1 𝑛 𝑖𝑛𝑖𝑡𝑖𝑎𝑙 2 )

What is the wavelength of a FM radio transmission at 88.9 MHz?

What is the frequency of light with a wavelength of 660 nm?

Ultraviolet radiation has a frequency of 6. 8 × 1015 s-1 Ultraviolet radiation has a frequency of 6.8 × 1015 s-1. Calculate the energy, in joules, of the photon.

A sodium vapor lamp emits light photons with a wavelength of 5 A sodium vapor lamp emits light photons with a wavelength of 5.89 × 10-7 m. What is the energy of these photons?

A ruby laser produces red light that has a wavelength of 500 nm A ruby laser produces red light that has a wavelength of 500 nm. Calculate its energy in joules.

What is the frequency of UV light that has an energy of 2.39 × 10-18 J?

Determine the de Broglie wavelength (in nm) associated with a neutron traveling at a speed of 5.0 x 103 m/s. The mass of a neutron is 1.67 x 10–24 g.

What is the wavelength of an electron moving at 5 What is the wavelength of an electron moving at 5.31 x 106 m/s if an electron has a mass of 9.11 x 10-31 kg?

An atom of helium has a de Broglie wavelength of 4. 30 x 10¯12 m An atom of helium has a de Broglie wavelength of 4.30 x 10¯12 m. What is its velocity?

Calculate the wavelength of the radiation emitted by a hydrogen atom when an electron falls from the n=3 to the n=2 orbital in the Bohr model.

What is the ionization energy of an electron in the n=3 shell of a hydrogen atom?

What is the molar absorptivity of the following compound as measured in a 1 cm cuvette? Concentration: 25uM Absorption: 0.5874

What is the concentration of the following compound as measured in a 1 cm cuvette: Molar absorptivity: 4525 M-1cm-1 Absorption: 0.6358

A student wishes to analyze the concentration of an unidentified yellow solution. What wavelength should be used to measure absorption?